CHEMISTRY 1
FINAL EXAM REVIEW 2013-2014
PAGE 1
1. Which of the following statements about ionic and covalent bonding is false?
(Ch. 12)
a. Covalent bonds are formed between atoms having high ionization energies.
b. Ionic bonding results in substances which form conducting solutions when dissolved in water.
c. In ionic bonding, atoms gain and lose electrons to obtain the same number as the nearest noble gas.
d. Covalent bonding can only happen between like atoms.
e. Covalent bonding may result in single, double or triple bonds.
2. The equation for the dissolving of Ba(NO3)2 in water is which of the following? (Ch. 12)
a. Ba(NO3)2(s)  Ba2+(aq) + 2 NO3-(aq)
b. Ba(NO3)2(s)  Ba2+(aq) + (NO3)2-(aq)
c. Ba(NO3)2(s)  Ba2+(aq) + (NO3)22-(aq)
d. Ba(NO3)2(s)  Ba(NO3)2(aq)
e. Ba2+(aq) + (NO3)2-(aq)
 Ba(NO3)2(s)
3. Which of the following statements about the visible part of the electromagnetic spectrum is not true? (Ch. 11)
a. The velocity of visible light is 3.00 x 108 meters/second.
b. The frequency of visible light can be found by the relationship ( = c/).
c. The higher the frequency of light, the greater its energy per photon.
d. The longer the wavelength of light, the greater its energy per photon.
e. Visible light is a very small part of the entire electromagnetic spectrum.
4. Which of the following statements about the quantum-mechanical model for the atom is not true? (Ch. 11)
a. Electrons exist only in shells which are a specific distance from the nucleus. This distance is determined by the
principal quantum number, n.
b. The principal quantum number, n, is used to describe the energy level in which an electron may be found.
c. For every principal quantum number, n, there are n2 orbitals available for electron occupancy.
d. It is often useful to consider the electron’s wave characteristics rather than its particle characteristics.
e. The quantum-mechanical model tells only the probability of finding an electron in a given area of space.
5. Which of the following formulas is not reasonable? (Ch. 11)
a.
SiO2
d.
NO
b.
Al2O3
e.
MgF2
c.
CO2
6. Positive ions are usually formed by which of the following processes? (Ch. 3, 11)
a. gain of protons by the nucleus.
b. loss of electrons from the nucleus.
c. loss of neutrons from the nucleus.
d. gain of electrons either inside or outside the nucleus.
e. loss of electrons from outside the nucleus.
7. Which of the following statements about the periodic table is false? (Ch. 3, 11)
a. Metals are generally located on the left side of the periodic table, and nonmetals on the right.
b. The elements are arranged in order of increasing atomic number.
c. Elements in each vertical column of the periodic table have similar chemical reactions.
d. Elements in each horizontal row have nearly identical physical characteristics.
e. Elements on the left side of the periodic table generally form positively charged ions when they react.
8. Which of the following will have the highest ionization energy? (Ch. 11)
a. Na
b. Al
c. Ca
d. Mg
e. H
CHEMISTRY 1
FINAL EXAM REVIEW 2013-2014
PAGE 2
9. Which of these electron configurations for neutral atoms in their lowest energy state is not correct? (Ch. 11)
a.
fluorine
1s12s22px22py22pz1
b.
rubidium
[Kr] 5s1
c.
scandium
1s22s22p63s23p64s24px1
d.
zinc
[Ar] 4s23d10
e.
germanium
[Ar] 4s23d104px14py1
10. The isotope 27Al contains ______ protons in its nucleus. (Ch. 3)
a. 13
b. 14
c. 27
d. 40
e. none of these
11. What is the energy of a photon of ultraviolet radiation,  = 5.00 x 10-8 m?
E = h and = c (h = 6.626 x 10-34 Js c = 3.00 x 108 m/s) (Ch. 11)
a.
1.11 x 10-49 J
d.
3.98 x 10-18 J
b.
1.67 x 10-16 J
e.
7.24 x 10-12 J
-33
c.
9.95 x 10 J
12. Which atom has the highest ionization energy? (Ch. 11)
a. Mg
b. Be
c. Ba
d. Ca
e. Sr
13. Which of the orbitals below has the highest energy? (Ch. 11)
a. 6s
b. 5p
c. 5s
d. 5d
e. 4f
14. Which element in the nitrogen family is most metallic? (Ch. 11)
a.
nitrogen
d.
antimony
b.
phosphorus
e.
bismuth
c.
arsenic
15. In 0.500 moles of acetic acid, CH3COOH, there are (Ch. 6)
a.
6.02 x 1023 molecules
d.
2.4 x 1024 atoms
23
b.
3.01 x 10 molecules
e.
4.8 x 1024 atoms
c.
1.8 x 1024 atoms
16. Once cubic millimeter is equal to a volume of (Ch. 5)
a.
1 mL
d.
b.
0.01 mL
e.
c.
100 mL
17. What is the mass of one platinum atom? (Ch. 6)
a.
1.6 x 10-22 g
b.
3.2 x 10-22 g
c.
5.13 x 10-3 g
0.001 mL
10 mL
d.195.08 g
e. none of these
18. Which is not true for covalent bonds? (Ch. 12)
a.
The pair of electrons is shared between the two atoms.
b.
More than two electrons can be shared between the two atoms.
c.
Covalent bonds usually do not break in aqueous solutions.
d.
One electron in the bond must come from each atom.
e.
Ionic bonds are about as strong as covalent bonds.
19. Which of the following molecules contains one triple bond? (Ch. 12)
a. NH3
b. CO
c. H2CCO
d. H2CCH2
e. HNNH
CHEMISTRY 1
FINAL EXAM REVIEW 2013-2014
20. Which of the following diatomic molecules has the greatest bond strength? (Ch. 12)
a. H2
b. F2
c. N2
d. O2
PAGE 3
e. HF
21. How many molecules are in 160 grams of nitrogen gas? (Ch. 6)
a.
6.9 x 1024
d.
9.6 x 1025
24
b.
3.4 x 10
e.
1.6 x 1023
c.
1.4 x 1025
22. What is the electron configuration of a stable magnesium atom? (Ch. 11)
a.
1s22s22p5
d.
1s22s22p63s2
2 2
6
b.
1s 2s 2p
e.
1s22s22p63s23p1
c.
1s22s22p63s1
23. The following species S2-, Cl-, Ar, K+ , all have the same number of (Ch. 3, 11)
a.
protons
d.
neutrons
b.
nucleons
e.
isotopes
c.
electrons
24. The neutral atoms of all the isotopes of the same element have (Ch. 3)
a.
different numbers of protons
b.
different numbers of neutrons
c.
the same number of electrons
d.
the same masses
e.
the same mass number
25. Which of the following is likely to have the largest radius? (Ch. 11)
a. H
b. Mn
c. Cl
d. Rb
e. Ag
26. Which property is not a characteristic of the alkali metals? (Ch. 11)
a.
Their chlorides are water soluble.
b.
They react with water to give off hydrogen gas.
c.
They can be found as the free element in nature.
d.
They are all reactive, readily losing one electron to form ions with a +1 charge.
e.
They all have the outer electron configuration ns1.
27. How many valence electrons are in the outer shell of a Pb atom? (Ch. 11)
a. 2
b. 3
c. 4
d. 5
e. 6
28. An element E has the electron configuration [Kr]4d105s25p2. The formula for the fluoride of E is most likely (Ch. 11)
c.
a. EF14
b. EF8
c. EF6
d. EF4
e. EF
29. Of the following elements, which needs three electrons to complete its valence shell? (Ch. 3, 11)
a. Ba
b. Si
c. Cl
d. Ca
e. P
30. Which of the following contains no ionic compounds? (Ch. 12)
a.
HCN
NO2
Ca(NO3)2
b.
PCl5
LiBr
Zn(OH)2
c.
KOH
CCl4
SF4
d.
NaH
CaF2
NaNH2
e.
CH2O
H2S
NH3
CHEMISTRY 1
FINAL EXAM REVIEW 2013-2014
PAGE 4
31. Aluminum has a density of 2.7 g/mL. How much volume will be occupied by 4.0 moles of aluminum? (Ch. 6)
a. 10. mL
b. 20. mL
c. 30. mL
d. 40. mL
e. 50. mL
32. What is the answer to the correct number of significant figures?
a. 0.38
b. 0.4
c. 0.3751
(0.0821)(0.023)(298) / 1.5 (Ch. 5)
d. 0.375
e. 0.37514227
33. Which electron configuration is impossible? (Ch. 11)
a.
1s22s22p63s2
b.
1s22s22p62d2
c.
1s22s22p63s23p6
d.
1s22s22p63s1
e.
1s22s22p63s23p64s1
34. Which pair is geometrically similar? (Ch. 12)
a.
SO2 and CO2
b.
PH3 and BF3
c.
CO2 and OF2
d.
SO2 and O3
e.
CO32- and NH3
35. A metal M, forms an oxide of formula M2O3. The ground state valence shell electron configuration of the M atom is:
(Ch. 12)
a.
ns2np1
d.
ns2
1
10
b.
4s 3d
e.
ns1
2
3
c.
ns np
36. Which ion is smallest in size? (Ch. 11)
a. Al3+
b. F-
c. O2-
d. Na+
e. N3-
37. If you take one mole of aluminum sulfate and break it up into ions, how many moles of ions are there per mole of
Al2(SO4)3? (Ch. 6)
a. 1
b. 2
c. 4
d. 5
38. The molecule CCl2F2 is expected to have what kind of geometry? (Ch. 11)
a.
bent
d.
trigonal planar
b.
tetrahedral
e.
pyramidal
c.
see-saw
39. An atom has in its nucleus 47 protons and 60 neutrons. What is the isotopic symbol for this element? (Ch. 3)
60
a.
Ag
107
b.
Nd
13
c.
Al
107
d.
Ag
40. If the following pairs of elements form ions, which pair would form an ionic compound of the general formula C2A
(where C = cation and A = anion)? (Ch. 3, 11)
a. sodium and sulfur
b. aluminum and oxygen
c. calcium and bromine
d. magnesium and sulfur
CHEMISTRY 1
FINAL EXAM REVIEW 2013-2014
PAGE 5
41. Reading from left to right across a row of the periodic table, the atomic radius becomes: (Ch. 11)
a. larger, owing to increased nuclear charge that is only partially shielded by additional valence electrons.
b. smaller, owing to increased nuclear charge that is only partially shielded by additional valence electrons.
c. smaller, owing to placement of additional electrons in more strongly bonding (closer) orbitals.
d. larger, owing to placement of additional electrons in more strongly bonding (closer) orbitals.
42. Which of the following shows atoms in expected order of increasing ionization energy? (Ch. 11)
I. Be, Mg, Ca
II. B, C, N
III. K, Na, Li
a. I only
b. II only
c. III only
d. II and III only
43. A sample of table sugar is found to have a mass of 61.45 grams and a volume of 38.72 cm 3. What is the density of
sugar, in grams per cubic centimeter? (Ch. 5)
a. 0.63
b. 1.06 x 10-3
c. 1.59
d. The density of a water soluble solid cannot be determined.
44. How many atoms of hydrogen are represented in the following formula?
(NH4)2CO3 (Ch. 3)
a. 4
b. 8
c. 24 x 1023
d. 48 x 1023
45. Which one of the following molar masses is not correct? (Ch. 6)
a. H2O = 18.0
d. H2S = 34.1
b. SO2 = 32.1
e. H2SO4 = 98.1
c. H2SO3 = 82.1
46. What is the molar mass of copper (II) nitrate? (Ch. 6)
a. 139.5 g
c. 171.5 g
e. 227.2 g
b. 157.5 g
d. 187.6 g
47. What is the mass, in grams, of 0.350 mole of silver nitrate? (Ch. 6)
a. 35.0 g
c. 76.4 g
e. 485 g
b. 59.5 g
d. 169.9 g
48. How many moles of copper are present in 7.50 g of copper? (Ch. 6)
a. 0.118 mole
d. 63.5 mole
b. 0.130 mole
e. 476 mole
c. 7.50 moles
49. How many moles of copper (II) sulfate are present in a 10.0 gram sample of the compound? (Ch. 6)
a. 0.0627 mole
d. 160 moles
b. 10.0 moles
e. 1.60 x 103 moles
c. 16.0 moles
50. Which of the following quantities represents the greatest mass of nitrogen gas (N2)? (Ch. 6)
a. 22.4 moles
d. 6.022 x 1023 molecules
b. 22.4 liters at STP
e. 1 molar weight in grams
c. 28.0 g
CHEMISTRY 1
FINAL EXAM REVIEW 2013-2014
PAGE 6
51. Which one of the following problems is answered to the correct number of significant figures? (Ch. 5)
a. 14.0/2 = 7.0
d. 14.0/2.0 = 7.00
b. 14.0/2.0 = 7
e. none of the above
c. 14.0/2 = 7
52. How many of the zeros in the measurement 0.000040200 meter are significant? (Ch. 5)
a. 2
b. 3
c. 7
d. 8
53. Choose the correct formula for magnesium phosphate (Ch. 4)
a. Mg3P2
b. MgPO3
c. Mg3(PO4)2
54. Choose the correct name for Li2CO3 (Ch. 4)
a. lithium carbonate
b. lithium (II) carbonate
d. lithium (II) carbide
e. dilithium tricarbonate
d. MgPO4
c. lithium carbonite
55. Concentrated hydrochloric acid has a density of 1.19 g/mL. What is the mass, in grams, of 2.00 liters of this acid?
(Ch. 5)
a. 2.38 x 103 g
c. 4.20 x 10-4 g
-3
b. 2.38 x 10 g
d. 4.20 x 104 g e. impossible to determine with this data
56. What is the volume, in liters, of 3.75 mole of oxygen gas at STP? (Ch. 6)
a. 3.75 L
c. 32.0 L
b. 84.0 L
d. 1.20 x 102L e. none of these
57. How many atoms are contained in a 12.5 gram sample of silver metal? (Ch. 6)
a. 6.97 x 1022 atoms
c. 7.52 x 1024 atoms
b. 0.116 atoms
d. 1.92 x 10-25 atoms
e. none of these
58. Which element when combined with chlorine would most likely form an ionic compund? (Ch. 12)
a. lithium
b. carbon
c. bromine
d. phosphorous
59. What is the ionic charge on the chromium ion in the ionic compound with the formula Cr2O3? (Ch. 3)
a. 3+
b. 2+
c. 2d. 3e. 6+
60. What is the molar mass of magnesium chloride? (Ch. 6)
a. 59.8 g
b. 95.2 g
c. 125.8 g
d. 76.4 g
61. How many significant figures should be reported for the product of
3.00 cm x 12.0 cm x 3.100 cm? (Ch. 5)
a. 1
b. 2
c. 3
d. 4
e. 5
62. What is the formula for diarsenic trioxide? (Ch. 4)
(a) As2O3 (b) As3O2 (c) As2(O2)3 (d) As3(O2)2
42 
63. The ion of potassium-42, 19
K contains (Ch. 3)
(a) 19 protons, 18 electrons, 22 neutrons
(b) 19 protons, 18 electrons, 23 neutrons
(c) 19 protons, 19 electrons, 23 neutrons
(d) 18 protons, 19 electrons, 24 neutrons
(e) 42 protons, 44 electrons, 19 neutrons
CHEMISTRY 1
FINAL EXAM REVIEW 2013-2014
PAGE 7
64. A physicist named J.J. Thomson showed that all atoms can be made to emit tiny particles which are repelled by the
negative pole of an electric field. Which subatomic particle was this evidence for? (Ch. 3)
a. proton
b. neutron
c. electron
d. nucleus
e. isotope
65. Some elements exist in nature as diatomic molecules. Which of the elements below will be found as diatomic
molecules? (Ch. 3, 12)
a) Ar
b)
O
c)
K
d) F
e)
S
f)
N
g) H
h)
Cl
66. Which of the following compounds will conduct an electric current? (Ch. 12)
a) NaCl (aq)
b) NaCl (s)
c) NaCl (l)
d) C12H22O11 (aq)
e) P4O10
f) both a & c
67. Name the following compounds: (Ch. 4)
a. FeCl3
b. AlP
c. SnF2
d. S2F10
e. CCl4
68. Balance these equations: : (Ch. 7)
Cu
+
Fe2S3
H2
H2SO4 

CuSO4
+
H2O + SO2
O2 

Fe2O3
+
SO2
+
+
Fe3O4


H2O
+
Fe
69. Write formulas for the following compounds: (Ch. 4)
a) cobalt (III) iodide
b) silver chloride
c) lithium nitride
d) dichlorine heptoxide
e) nitrogen dioxide
70.
71.
What is the half-life of Mo-88? (Ch. 19)
a. 16 minutes
b. 14 minutes
c. 8 minutes
d. 7 minutes
Looking at the graph above, at what time would 75% of the Mo-88 be decayed? (Ch. 19)
a. 16 minutes
b. 14 minutes
c. 8 minutes
d. 7 minutes
CHEMISTRY 1
FINAL EXAM REVIEW 2013-2014
PAGE 8
Use this information for the next three questions. A strip of metallic zinc, Zn, was weighed and placed in a beaker
containing a solution of silver nitrate, AgNO3. The next day, a silvery metallic deposit was present in the beaker. The zinc
strip was washed, dried and weighed. The liquid was decanted off the metallic residue which was also washed, dried and
weighed. The data obtained are recorded below:
Mass of zinc before reaction = 14.26 g
Mass of zinc after reaction = 13.61 g
Mass of silver produced = 2.16 g
72. How many moles of zinc reacted? (Ch. 6)
a. 0.010 mole
b. 0.0200 mole
c. 0.0500 mole
d. 0.100 mole
e. 0.200 mole
73. How many moles of silver were formed? (Ch. 6)
a. 0.010 mole
b. 0.0200 mole
c. 0.0500 mole
d. 0.100 mole
e. 0.200 mole
74. The reaction which took place can be written in the following form:
_____ zinc (solid) + _____ silver nitrate (in solution) 
 _____ silver (solid) + _____ zinc nitrate (in solution).
The coefficients for the substances in the above equation are, in order of appearance: (Ch. 6)
a. 1,1,1,1
b. 2,1,1,2
c. 1,2,2,1
d. 1,3,3,1
e. 2,3,3,2
75.
This diagram represents (Ch. 19)
a) a fission reaction.
b) a fusion reaction.
76.
c) spontaneous radioactive decay.
d) electron capture.
What is the second product in the diagram above? (Ch. 19)
a) 143
b) 142
54 Xe
54 Xe
c)
145
54
Xe
77.
The half-life of radioactive atoms refers to (Ch. 19)
a. Half the time required for all atoms in a sample to disintegrate.
b. The number of atoms that decay in half a second.
c. The number of atoms in a sample that are radioactive.
d. The time required for half the atoms in a sample to disintegrate.
78.
The greatest penetrating power is associated with the type of radiation called (Ch. 19)
a. alpha particles
b. beta particles
c. gamma rays
d. x-rays
79.
The radiation originally labeled as alpha is now known to be made up of (Ch. 19)
a. Helium nuclei
b. electrons
c. positrons
d. gamma rays
CHEMISTRY 1
80.
FINAL EXAM REVIEW 2013-2014
What is the particle emitted in the nuclear change given by the following equation? (Ch. 19)
234
91
Pa 

234
92
U + __________
a. an alpha particle
81.
PAGE 9
b. a beta particle
c. a neutron
d. a positron
In the nuclear equation
288
92
U 

B
A
X + 42 He
The letters A and B, are respectively (Ch. 19)
a. 90 and 242
b. 94 and 242
c. 94 and 234
d. 90 and 234
82. What is the particle emitted when aluminum is changed to phosphorous by bombarding the aluminum with alpha
particles, as shown by the equation? (Ch. 19)
27
13
Al + 42 He 

a. Proton
30
15
P + _________
b. positron
c. neutron
83. The relatively high penetrating power of neutrons is due to their (Ch. 19)
a. Small size
b. high speed
c. lack of charge
d. large mass
84. The term transmutation refers to the (Ch. 19)
a. Gain of energy as a result of mass loss.
b. Change of one compound into a new compound.
c. Gain or loss of electrons by neutral atoms.
d. Change of one element into an entirely different element.
85. Which element is an alkali metal? (Ch. 11)
a. K
b. Cl
c. Mg
d. Cu
d. As
86. Which element is a metalloid? (Ch. 11)
a. K
b. Cl
c. Mg
d. Cu
d. As
87. Which element has the highest electronegativity? (Ch. 11)
a. K
b. Cl
c. Mg
d. Cu
88. Convert (Ch. 5)
a. 4.32 mm to pm
b. 75.00 g to kg
d. As
d. 8.5 x10-3 L to mL
c. 432 nm to m
89. In a molecule of (NH4)2SO4, how many oxygen atoms are there? (Ch. 4)
Nitrogen atoms?
Sulfur atoms?
Hydrogen atoms?
90. Draw the Lewis dot structure for:
a. Mg
b. N
c. CO2
d. SO2
e. CCl4